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2 years ago

Will mark as Brainliest.

Chemistry

2 answers:

kifflom [539]2 years ago

7 0

You’re going to need to use stoichometry to solve this. Hope this helps

postnew [5]2 years ago

3 0

<span>0.453 moles O2 is the solution</span>

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Need Help ASAP

bagirrra123 [75]

a. pH=2.07

b. pH=3

c. pH=8

<h3>Further explanation</h3>

pH=-log [H⁺]

a) 0.1 M HF Ka = 7.2 x 10⁻⁴

HF= weak acid

$\tt [H^+]=\sqrt{Ka.M}\\\\(H^+]=\sqrt{7.2.10^{-4}\times 0.1}\\\\(H^+]=8.5\times 10^{-3}\\\\pH=3-log~8.5=2.07$

b) 1 x 10⁻³ M HNO₃

HNO₃ = strong acid

$\tt pH=-log[1\times 10^{-3}]=3$

c) 1 x 10⁻⁸ M HCl

$\tt pH=-log[1\times 10^{-8}]=8$

5 0

2 years ago

Which metal is more active than H2?<br> (1) Ag (3) Cu<br> (2) Au (4) Pb

astraxan [27]

Answer is (4) - Pb.

According to the reactivity series of elements

- the elements which are above the hydrogen are more reactive than hydrogen.

- the elements which are below the hydrogen are less reactive than hydrogen.

Among the given choices, only Pb is placed above the hydrogen in the reactivity series and rest are below the hydrogen.

Hence, Pb is more active than hydrogen.

5 0

2 years ago

Difference between a row (“period”) & a column (“group”) on the periodic table and examples.

saw5 [17]

The rows are the one line of elements that goes from left to right horizontally. A column is a line of elements that goes vertically.

5 0

2 years ago

Read 2 more answers

Ignore, question was removed

djverab [1.8K]

Rip bro but I need the point

6 0

2 years ago

A 4.36 g sample of an unknown alkali metal hydroxide is dissolved in 100.0 ml of water. an acid-base indicator is added and the

Fofino [41]

Answer:

(a) $102.6g/mol$

(b) Rubidium

Explanation:

Hello,

This titration is carried out by assuming that the volume of base doesn't have a significant change when the mass is added, thus, we state the following data a apply the down below formula to compute the molarity of the base solution:

$V_{base}=0.1L; M_{acid}=2.5M, V_{acid}=0.017L\\V_{base}M_{base}=V_{acid}M_{acid}$

Solving for the molarity of base we've got:

$M_{base}=\frac{M_{acid}*V_{acid}}{V_{base}}=\frac{2.50M*0.017L}{0.1L} =0.425M=0.425mol/L$

Now, we can compute the moles of the base as:

$n_{base}=0.425mol/L*0.1L=0.0425mol$

(a) Now, one divides the provided mass over the previously computed moles to get the molecular mass of the unknown base:

$\frac{4.36g}{0.0425mol} =102.6g/mol$

(b) Subtracting the atomic mass of oxygen and hydrogen, the metal's atomic mass turns out into:

$102.6g/mol-16g/mol-1g/mol=85.6g/mol$

So, that atomic mass dovetails to the Rubidium's atomic mass.

Best regards.

8 0

2 years ago